Question

A rigid plastic container holds 1.00 l methane gas at 660 torr pressure when the temperature is 22.0 degrees Celsius. How much pressure will the gas exert if the temperature is raised to 44.6 degrees Celsius?

Answer 1

 PV/T = P'V'/T' 
660 x 1.00/295.2 = P' x 1.00/317.8 
P'=710.5 torr

Answer 2

Answer : The final pressure of the gas will be, 710.56 torr

Explanation :

According to the Charles' Law, the pressure of the gas is directly proportional to the temperature of the gas at constant volume and the number of moles of gas.

$P\propto T$

or,

$\frac{P_1}{P_2}=\frac{T_1}{T_2}$

where,

$P_1$ = initial pressure of the gas = 660 torr

$P_2$ = final pressure of the gas = ?

$T_1$ = initial temperature of the gas = $22^oC=273+22=295K$

$T_2$ = final temperature of the gas = $44.6^oC=273+44.6=317.6K$

Now put all the given values in the above formula, we get the final pressure of the gas.

$\frac{660torr}{P_2}=\frac{295K}{317.6K}$

$P_2=710.56torr$

Therefore, the final pressure of the gas will be, 710.56 torr